Method of preparing magnesium hydroxide

ABSTRACT

METHOD OF PREPARING MAGNESIUM HYDROXIDE. AN AQUEOUS SOLUTION OF MAGNESIUM CHLORIDE IS REACTED WITH PARTICULATED QUICKLIME IN A SPECIFIED MOLAR RATIO IN A CLOSED ROTATED REACTION ZONE. THE PH OF THE REACTION MASS IS MAINTAINED AT A VALUE OF ABOUT 8 TO 8.5 WHILE THE REACTION IS PERFORMED AT A TEMPERATURE OF ABOUT 50-70*C. THE AQUEOUS MAGNESIUM CHLORIDE SOLUTION CONSISTS PREFERABLY OF BITTERN OBTAINED AS THE MOTHER LIQUOR IN THE PREPARATION OF COMMON SALT FROM SEA WATER.

June 25., 1974 HIsANQBU TABATA FI'AL '3,819,803

I METHOD OF PREPARING MAGNESIUM HYDROXIDE Original Filed June 15, 1970 6 Sheets-Sheet 2 June 25, 1974 IH|SANQBU TABATA E'T'AL 3,819,803

METHOD OF PREPARING MAGNESIUM HYDROXIDE Original Filed June 15, 1970 I 6 Sheets-Sheet 3 FIG. 3

Relation between the concentration of magnesium chloride and the purity of magnesium hydroxide obtained Mixing ration---------- .............CqO2MgQ=130.95 Effective lime Reaction temperature 60C Reaction time --3 hrs.

CaO/ g h 0.6 Purity June 25,1974

Original Filed June 15, 1970 Purity METHOD-OF PREPARING MAGNESIUM HYDROXIDE Flez.

Relation between the reuctibn temperature and the filtration time.

6 Sheets-Sheet t Mixing ratio CuO:MgO=t10.95

. v A H207, Reaction time --3 hrs.

Temp C' June 25, 1974 HRSANOBU TABATA ETAL 3,319,303

METHOD OF PREPARING MAGNESIUM HYDROXIDE Original Filed June 15, 1970 6 Sheets-Sheet 5 -FIG.5

Relation between the mixing ratio and the purity of magnesium hydroxide obtained Effective lime -95/. Reaction temperature --60'C Reaction time 3 hrs.

Purity Mixing ratio Ca: Mg in mol June 25, 1974 H|SANQBU T ETAL 3,819,803

METHOD OF PREPARING MAGNESIUM HYDROXIDE Original Filed June 15, 1970 6 Sheets-Sheet (5 F I G. 6

Relation between the reaction time and the purity of magnesium hydroxide obtained Mixing rutio---- CclO MgO=i:0.95 Effective lime 95% Reaction temperatu---- 57C CaO AAgO Purity Time in hrs.

United States Patent Othce 3,819,803 Patented June 25, 1974 3,819,803 METHOD OF PREPARING MAGNESIUM HYDROXIDE Hisanobu Tabata and Norimasa Tabata, both of 968 Kou, Ohgoshi-machi, Sakaide-shi, Kagawa-ken, Japan, and Rokuro Nakajima, deceased, late of Sakaide-shi, Japan, by Tama Nakajima, heir, 1831 Ohyabucho, Sakaideshi, Kagawa-ken, Japan Original application June 15, 1970, Ser. No. 46,286, now Patent No. 3,676,067. Divided and this application Apr. 20, 1972, Ser. No. 245,777

Claims priority, application Japan, June 19, 1969, 44/ 48,416, 44/48,417 Int. Cl. C01f 5/22 US. Cl. 423-160 4 Claims ABSTRACT OF THE DISCLOSURE Method of preparing magnesium hydroxide. An aqueous solution of magnesium chloride is reacted with particulate quicklime in a specified molar ratio in a closed rotated reaction zone. The pH of the reaction mass is maintained at a value of about 8 to 8.5 While the reaction is performed at a temperature of about 50-70 C. The aqueous magnesium chloride solution consists preferably of bittern obtained as the mother liquor in the preparation of common salt from sea water.

CROSS-REFERENCE TO PRIOR APPLICATION This is a division of copending application Ser. No. 46,286, filed June 15, 1970, now US. Pat. No. 3,676,067.

\ SUMMARY OF THE INVENTION 'Co-pending application Ser. No. 46,286, now Pat. No. 3,676,067, of which the present application is a division, relates to a method of manufacturing fresh water and concentrated brine or salt water from sea water by evaporating therefrom the scale forming component, calcium sulphate. To remove calcium sulphate, magnesium hydroxide is precipitated from the bittern obtained as a byproduct in the manufacture of common salt, and is converted to magnesium carbonate which is added to the sea water to precipitate calcium sulphate contained therein as calcium carbonate and filtered off.

The present invention relates to a method of manufacturing magnesium hydroxide usable in making fresh water and concentrated brine.

The conventional method of making fresh water and brine from sea water is to evaporate sea water either after acidifying it with acid and adding a reagent to prevent the precipitation of calcium sulphate, or after precipitating calcium sulphate directly therefrom by the addition of a seed to accelerate its precipitation.

Undesirably, these methods have serious drawbacks.

In the former method, in order to prevent the precipitation of calcium carbonate and calcium hydroxide in the early stage of concentration, sea water is acidified until its pH value reaches about 4, and a reagent, chiefly consisting of phosphate, is added to prevent the precipitation of calcium sulphatenBecause the solution has a pH of about 4, the equipment used must be acidresistant. Moreover, as the reagent which prevents the precipitation of calcium sulphate decomposes at higher temperatures, high temperature treatment is impossible. As the efficiency of this reagent decreases with the increase of the concentration of sea water during operation, the upper limit of possible concentration is about 6 B., and further concentration is almost impossible by this method.

The latter method is to add calcium sulphate as a seed for its precipitation, and to prevent the formation of scale on the heat conducting surface by growing calcium sulphate on the surface of its seed. However, calcium sulphate has several forms and is very sensitive to temperature and to the concentration of the sea water. For seeding'purposes it is necessary to select calcium sulphate of the same form as is deposited in the course of concentration which varies according to the conditions, and the seed must be very fine and ungrown. Moreover, to be effective, the amount of seed must be as much as 5-10% of the calcium sulphate contained in the sea water. As a result, the process is very difficult to control and as the amount of seed is considerable, the flow velocity required to evaporate the sea water in the heat conducting tube must be high. Accordingly, the evaporation efiiciency becomes very low. The method can hardly be adopted with multistage evaporators with varying temperatures such as flash evaporators.

While the concentrated brine obtained by these methods must further be evaporated in order to obtain common salt, the evaporation must be carried out with the addition of bittern to prevent the formation of scale. However, the addition of bittern raises the boiling point of the brine, and as the heat efiiciency in the evaporation is decreased, the equipment used must be large.

. The invention of the parent case relates to a method of manufacturing fresh water and brine from sea water wherein a 2-3% aqueous suspension of magnesium hydroxide obtained by the reaction between the bittern obtained as a by-product in the manufacture of common salt and quicklime is contacted with carbon dioxide previously purified by washing with a portion of said magnesium hydroxide liquor to form magnesium carbonate with a composition of CO :MgO=1:1.20-0.95 in mol; the magnesium carbonate is added to the sea water in the rates Ca++:CO "-=1:1.2 to the Ca++ contained in sea water to precipitate calcium sulphate as calcium carbonate; and the sea water purified in this way is concentrated, after filtration, by evaporation to obtain fresh water and brine.

The present invention relates to a process for producing magnesium hydroxide usable in the production of fresh water and concentrated brine from sea water, which comprises reacting a solution of magnesium chloride directly with quicklime. More practically, the present invention is a method of manufacturing magnesium hydroxide with high purity in which a concentrated solution of magnesium chloride, by-produced during the treatment of the sea water for example, is charged together with quicklime in lump (or pellet) form, in a closed vessel containing steel balls, the quicklime is ground by rotating said vessel, and the ground quicklime is reacted step by step with magnesium chloride to obtain magnesium hydroxide.

The invention now will be described in detail reference being made to the attached accompanying drawings in which:

FIG. 1 is a schematic diagram showing the process of producing fresh water and brine according to the invention of the parent case;

FIG. 2 is a schematic view of apparatus suitable for use in the method of the invention;

FIG. 3 is a graph showing the relationship between the concentration of magnesium chloride and the purity of magnesium hydroxide obtained;

FIG. 4 is a curve which shows the relationship between the reaction temperature and the filtration time;

FIG. 5 shows the relation between the mixing ratio and the purity of magnesium hydroxide obtained; and

FIG. 6 is a curve which shows the relation between the reaction time and the purity of magnesium hydroxide obtained.

The process of treating sea water will be explained by referring to FIG. 1. The bittern obtained as a byproduct in the manufacture of common salt and the like is reacted with quicklime to obtain magnesium hydroxide; carbon dioxide is absorbed in an aqueous suspension of said magnesium hydroxide to form magnesium carbonate; the magnesium carbonate is added to sea water to precipitate calcium sulphate dissolved in sea water as calcium carbonate, and the precipitate is filtered off and the purified sea water is concentrated in a flash evaporator or other evaporator, or by ion exchange to obtain fresh water and brine. The bittern obtained as a by-product in the further treatment of this brine may be recycled to the first stage of this invention to improve the economics of the process.

The prior art method of manufacturing magnesium hydroxide by reacting calcium hydroxide obtained by slaking quicklime with a solution of magnesium chloride has several disadvantages.

(1) To obtain calcium hydroxide, it is necessary to slake quicklime with water, and calcium hydroxide so obtained must be separated from coarse impurities, for instance, by passing through a sieve. As a result, the yield of calcium hydroxide is low.

Additionally, calcium carbonate is formed by the reaction of lime with carbon dioxide dissolved in water thereby decreasing the purity of the product. To manufacture magnesium hydroxide with high purity, it is necessary to first remove carbon dioxide from the water used for slaking, and to carry out the process of slaking in a closed vessel to prevent the contamination by carbon dioxide. As a practical matter, since the process of purifying the slaked lime is carried out in an open air, the formation of calcium carbonate cannot be avoided. Depending on the purity of the raw material, the loss of calcium oxide reaches as high as (2) It is necessary to heat the charge when reacting the slaked lime with a solution of magnesium chloride. Moreover, as the reaction does not go to completion leaving unreacted calcium hydroxide in the product, the purity and the yield of the product are decreased.

(3) Similarly with the prior art method, it is important to control the pH during the reaction. If the amount of calcium exceeds the amount of magnesium even for a short time, the precipitated magnesium hydroxide becomes colloidal, these colloidal particles absorb Ca++, and the magnesium hydroxide becomes impure. At the same time, the filtration and the washing of the magnesium hydroxide in the following stage becomes difficult. Therefore, it is necessary to charge magnesium chloride solution and milk of lime simultaneously, and to carefully control the pH in order to prevent even a momentary excess of calcium hydroxide. Practically, for instance, a 10% solution of magnesium chloride and a 17% milk of lime solution are charged simultaneously at 70 C. for 6 hrs., and after agitating further for 2 hrs. the mixture is filtered to obtain magnesium hydroxide.

However, as the particles of magnesium hydroxide obtained in this method are very fine, filtration and washing are difficult. As the calcium chloride solution obtained as a mother liquor of the reaction is dilute, the solution must be concentrated by heating in order to recover and to utilize calcium chloride.

For these reasons it is necessary in this prior method to use large scale equipment such as slaking, refining and heating devices. The purity of the product is not satisfactory and the method is costly.

An object of this invention is to provide an advantageous method of manufacturing high purity magnesium hydroxide. In accordance with this object an aqueous solution of magnesium chloride and quicklime in lump form are charged in a ratio of 1:0.9-0.95 calculated as MgOzCaO in mol, in a closed vessel containing steel balls, the closed vessel is rotated, and the reaction is completed by main taining the pH of the charge at 8.0-8.5.

As seen from FIG. 3 which shows the relation between the purity of magnesium hydroxide and the concentration of magnesium chloride at 60 C., it is desirable to use a 7-23% aqueous magnesium chloride solution for the reaction. Moreover, when the magnesium chloride concentration is under 7%, it is difiicult to raise the reaction temperature sufficiently high in practical operation; the reaction is incomplete and the purity of the product becomes unsatisfactory, containing unreacted raw materials. The reaction proceeds also slowly when the concentration is over 25%, and this is similarly undesirable.

Raw bittern, obtained as a mother liquor in the manufacture of common salt from sea water, contains about 20-26% of magnesium chloride together with about 10% of magnesium sulfate. When this raw bittern is treated with calcium chloride to remove the sulfate as calcium sulfate, it becomes a convenient source of magnesium chloride for this invention, directly or diluted to some extent.

As shown in FIG. 4, the filtration of the product can most readily be effected when the reaction temperature is about 50-70 C. This fact indicates that the particles formed are well crystallized, having a relatively large diameter of about 5011.. The optimum reaction temperature lies in this range. When the magnesium chloride concentration is about 723%, the reaction temperature can be maintained at about 50-70 C., although dilfering somewhat from the reaction conditions mentioned below.

It is desirable that the lump size of the quicklime used in this invention be mainly of a diameter of about 5-20 cm., with less than 50% powder. When the quicklime contains more than 50% powder, the reaction proceeds rapidly and the pH increases. When the pH exceeds 10.5 even for a moment, the precipitated magnesium hydroxide becomes colloidal, absorbs Ca++ and becomes impure. The formation of colloidal magnesium hydroxide should carefully be prevented.

It is desirable to select the mixing ratio of magnesium chloride solution and quicklime to be 1:0.9-0.95 calculated as MgOzCaO in mol. As seen from FIG. 5, magnesium hydroxide becomes impure outside this range, chiefly owing to the contamination by unreacted lime. From the standpoint of process control and operation cost etc., it is desirable that the mixing ratio be as close to 0.95 as possible.

The reaction is carried out in a closed vessel. It is desirable that the free space in the vessel be as small as possible in chargingv the reaction mixture in order to prevent the formation of calcium carbonate due to the carbon dioxide in air.

The reaction vessel is rotated to grind quicklime in lump form gradually and to react the pulverized quicklime slowly with magnesium chloride, maintaining the pH of the charge within the range of 8.0-8.5. The rotation speed of the reaction vessel is controlled in accordance with conditions, such as the number and size of the steel balls, to maintain the pH in the desired range of 8.0-8.5 and to finish the reaction in about 3 hrs. Under these conditions, the reaction temperature can be maintained at the optimum of about 50-70 C. as previously stated.

The closed reaction vessel consists of a steel rotary vessel which contains steels balls having a diameter of about 10 cm. The number of steel balls as well as the rotation of the vessel are selected so as to satisfy the reaction conditions above-mentioned.

Quicklime in lump form can be used for the reaction. As the quicklime in lump form is ground gradually by the steel balls in the closed reaction vessel and is reacted slowly with magnesium chloride, there is no danger of sudden temperature rise or of rapid pH increase. Therefore, the precipitated magnesium hydroxide crystallizes well in relatively large particles of high'purity, without forming colloidal particles, and accordingly the finishing of the product filtration and washing, can be effected quite readily. Further, as concentrated calcium chloride is obtained as a mother liquor in the reaction between quicklime and magnesium chloride, its recovery is also quite economical, consuming only a small amount of heat for its further concentration.

The details of this invention will be illustrated by the following examples.

Bittern obtained in manufacturing common salt from brine or the brittern obtained by the common process is first treated with quicklime to obtain magnesium hydroxide. It is desirable that the magnesium hydroxide be very pure and has a relatively coarse particle size of about 50 The Mg(OI-I) is prepared as follows:

An aqueous 7-23,% magnesium chloride solution (bittern) and quicklime in lump form, mainly of a particle size of 5-20 cm. in diameter are charged, in a ratio of l:0.9-0.95 calculated as MgOzCaO, into a closed vessel containing steel balls, the closed vessel is rotated, and the reaction is effected by maintaining the pH of the charge at 8.0-8.5. The magnesium hydroxide obtained is very pure, and its washing and filtration in the following stage are very easy.

Then magnesium carbonate is manufactured by absorbing carbon dioxide in said magnesium hydroxide. In the prior art, the carbon dioxide from the calcination of magnesite, limestone or dolomite (18-25%) was used. The gas was freed from dust, washed with water and absorbed in an absorption tower under a pressure of 2-3 kg./cm. g. to manufacture magnesium carbonate. However, in this procedure, waste combustion gas such as boiler gas is used as the source of carbon dioxide. In a 23% aqueous liquor of magnesium hydroxide obtained in the previous stage, the gas is absorbed after washing with a portion of said aqueous magnesium hydroxide liquor. Not only the cost of the carbon dioxide material is almost zero, but also the process is air pollution free.

EXAMPLE 1 Manufacturing Fresh Water and Brine As shown in FIG. 2, (1) is a storage tank containing about one half (volume) of the aqueous 2-3% magnesium hydroxide suspension, and the suspension is pumped from the bottom of this tank to a pressure washing tank (4) through an ejector with the aid of a pump (2). An ejector (3) sucks combustion gas at the same time, and the gas is washed with the suspension. This gas liquid ejector (3) is fitted at the top of the pressure washing tank, and the tank (4) consists of a closed vessel with, for example, a diameter of 800 mm. and a height of 2000 mm. A crude combustion gas or boiler gas is sucked through a pipe (5) by the ejector (3), washed sufficiently with the liquid and enters in the tank (4). As the tank (4) is closed, its inner pressure becomes about 0.4 kg./cm. g., and the gas is separated from the liquor in this tank. The gas purified by washing is blown, as shown in-the figure, through a pipe into an absorption tower (7) from its bottom in the form of bubbles.

The magnesium hydroxide liquor in the tank (4) used for the washing of the gas is circulated through a pipe (6) to the tank (4), and is renewed occasionally when the liquor becomes contaminated.

The absorption tower (7 contains an aqueous 2-3% magnesium hydroxide suspension to a height of 4 m., and this magnesium hydroxide is carbonated with the carbon dioxide gas coming from tank (4) to give magnesium carbonate. Magnesium carbonate so obtained flows out together with the mother liquor from pipe (8) at the top of the tower. In the figure, (9) is a tank containing a 2-3% aqueous magnesium hydroxide suspension which is pumped to the tower (7) through a pressure pump (10). In the absorption tower (7 a gas distribution plate (11) and pipes are provided to accelerate the reaction while (13) is a wire netting to support the pipes (12). The result of a run using this equipment is as follows: a 1.5 kw. circulation pump with a working capacity of T/hr., an ejector with a nozzle diameter of 14 mm. were used, and a boiler waste gas with a carbon dioxide concentration of 13.5% was sucked. A 2% aqueous magnesium hydroxide suspension was used as an absorption liquor with a flow rate of 400 l./hr., and 12 kg. of pure basic magnesium carbonate was obtained per hour. The

Has 0 4 for pH Ca MgGOa control Mg(OH)rconcentration removal concen- (cc/kl. sea (percent) COQIMgO (percent). tratlon water) 1 As the concentration of magnesium carbonate is dilute, the amount of water to be evaporated becomes large.

The conventional method of purifying combustion gas such as waste boiler gas by washing arid the method of manufacturing magnesium carbonate by using the purified gas is as follows: Ash and dust of the gas are removed first through a dust collector, then the gas is washed through a washing tower, and is absorbed in an aqueous magnesium hydroxide suspension in an absorption tower to obtain magnesium carbonate. In that method, a costly high power compressor is needed to operate a dust collector and a washing tower. Moreover, as a continuous operation for a long time is almost impossible due to the adhesion of scale contained in the carbon dioxide on the surface of the valve of compressor and the like, it is usual to provide a spare compressor and to use them alternately. The power consumption is thus large and careful process control is required. Moreover, as carbon dioxide is diluted due to its solution in the large amount of water necessary for the washing, it is necessary to increase the pressure of the gas to compensate for its dilution.

The present procedure eliminates these drawbacks. By using an ejector, the three operations of suction, washing and compression of carbon dioxide can be carried out in one step. Therefore, the compression pressure is low enough, and only one pump is needed for the circulation of the driving liquor of the ejector. As the wash liquor of the gas is circulated as the driving liquor of the ejector, only a small amount of wash liquor is necessary. Moreover, as the concentration of carbon dioxide is always almost constant, process control is quite simple, and it is possible to manufacture high purity magnesium carbonate. v v

The material balance for the present method is compared below with that of the conventional method. To obtain 100 kg. magnesium carbonate the comparison is:

An aqueous magnesium carbonate suspension with the composition of CO :MgO=1.20-0.95 obtained in the above process was added without filtration, to sea water to react with Ca++ dissolved in sea water in an amount of Ca++/CO =l.2. When the reaction was carried out at 40 C. for 3 hrs. under stirring, the removal of calcium after filtration was 98%. The purified sea water was neutralized to pH 7 with sulphuric acid, deaerated, and conveyed to a flash evaporator. When 20.6 kl. of the purified sea water was evaporated in a flash evaporator, 4.3 kl. of the brine with a concentration of 15 B. was obtained together with 16.34 kl. of fresh water. Similar re sults were obtained by using magnesium carbonate after separation, or by using a common evaporator or by ion exchange.

The fresh water obtained was very pure, containing only less than 20 ppm. of chlorine, and was suitable as drinking water or for use in boilers. Heavy water was concentrated in this brine, and on further concentration the content of heavy water in 34 B. bittern was 0.28%, and in more concentrated bittern, 0.34%.

EXAMPLE 2 Production of Magnesium Hydroxide To a closed vessel of a cylindrical rotary drum with a diameter of 750 mm., a length of 750 mm. and a capacity of 400 1. containing 20 steel balls with a diameter of cm., 35 kg. of quicklime in lump form with a diameter of 10-20 cm. and 300 l. of a 20% aqueous magnesium chloride solution were charged. There was almost no free space in the vessel.

The closed Vessel was rotated 30 times per minute. Quicklime in lump form was ground gradually by the steel balls and reacted slowly with magnesium chloride. No sudden increase of the pH was observed, maintaining the pH of 8.0-8.5. The reaction temperature was almost constant at about 60 C. After reacting for 3 hrs., the product was filtered through a belt filter. After washing, the magnesium hydroxide product had a particle size of about 50p. and was very pure.

The relation between reaction time and the purity of magnesium hydroxide obtained in the same condition as above-mentioned is shown in FIG. 6. Although the reason is not certain, the product after 3 hrs. was purest.

The results are compared below with those of the conventional method under similar condition.

sea water, treated at 60 C., for 3 hrs. to precipitate Ca as calcium carbonate, and filtered. 98% of Ca++ in sea Water was removed. 20.6 kl. of the mother liquor was deaerated, its pH was brought to 6.5 with sulphuric acid, and was evaporated in a flash evaporator. 3.4 kl. of 15 B. brine was obtained, and the chlorine content of the fresh water distilled was only 20 p.p.m. Heavy water was concentrated in the brine, and on further concentration the content of heavy water in 34 B. was 0.28%, and in more concentrated bittern, 0.34%.

After 10 days of continuous operation by the flash evaporator, no scale formation was observed.

As above-mentioned, the present invention offers an economic method of treating sea water, in which magnesium carbonate suitable for the reaction is manufactured advantageously, from magnesium hydroxide, and from the bittern obtained as a by-product in the manufacture of common salt from sea water, the sea water is purified by treatment with magnesium carbonate and evaporated with a high heat efficiency and without the formation of scale to obtain the brine, which can further be concentrated to manufacture common salt without the addition of bittern, together with very pure fresh water.

What is claimed is:

1. A method for preparing magnesium hydroxide which comprises reacting an aqueous solution of magnesium chloride with particulate quicklime which is, in part, in the shape of lumps having a diameter of 5 to 20 cm., and partially in powder form, the powder constituting less than 50% of the total amount, by mixing the magnesium chloride solution and quicklime in a closed vessel, said mixing being carried out at a rate to maintain the temperature of the reaction mixture at about 50 to 70 C.,

C onsumed at- Charged at- Reactlon Aqueous Electric C30 MgClz CEO: time caClg Vapor power For 100 kg. Mg (OH): (kg.) (kg) MgO (hrs.) Obta g) (kwh.)

Method of this invention 100 177 0. 5:1.0 3 858(20%) 0 12 Conventional method 120 199 0. 5:1.0 8 2,500(7%) 1,050 80 EXAMPLE 3 Production of Magnesium Hydroxide As in Example 2, an aqueous magnesium chloride solution and qiucklime were charged to the closed vessel which contained steel balls, the vessel was rotated with a revolution of 15 times per min. for 3 hrs. Substantially the same result was obtained as in Example 2.

The method of this invention offers excellent results in combination with the process of treating sea water to obtain common salt, for instance, as shown in FIG. 6.

Relatively concentrated bittern, obtained as a by-prodnet in the treatment of sea water to manufacture common salt was used as the source magnesium chloride in this invention. High purity magnesium hydroxide, obtained by the reaction between this bittern and quick lime according to this invention, was made to a 2-3% milk of magnesia, and was converted to magnesium carbonate by introducing carbon dioxide previously washed with a portion of the same milk of magnesia. This magnesium carbonate was added to sea water, in amount of Ca++:CO =1:1.2 based on the dissolved Ca++ in References Cited UNITED STATES PATENTS 7/1938 Mastin 423163 1/1964 Nikolai 423163 OSCAR R. VERTIZ, Primary Examiner B. E. HEARN, Assistant Examiner US Cl. X.R. 423-158, 164 

